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Osmotic Pressure

The solution ...

Question

The solution exhibiting an osmotic pressure of $2.4 a t m$ at $127^{\circ} C$ contains $12 g$ of an organic compound per litre of the solution .
Calculate the molecular mass of the organic compound.

82.1 g m o l^{- 1}

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164.2 g m o l^{- 1}

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246.3 g m o l^{- 1}

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328.4 g m o l^{- 1}

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Solution

The correct option is B $164.2 g m o l^{- 1}$
Osmotic pressure:

$π = \frac{n}{V} \times R T$

Here n is number of moles

$n = \frac{Given mass}{Molar mass} = \frac{w_{B}}{m_{B}} = \frac{12}{m_{B}}$

$V = 1 L R = 0.0821 L a t m m o l^{- 1} K^{- 1} T = 127^{\circ} C = 400 K$

$\Rightarrow π V = \frac{w_{B}}{m_{B}} \times R T m_{B} = \frac{w_{B} \times R \times T}{π \times V}$

$m_{B} = \frac{12 g \times 0.0821 L a t m m o l^{- 1} K^{- 1} \times 400 K}{2.4 a t m \times 1 L} m_{B} = 164.2 g m o l^{- 1}$

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